Respuesta :
Answer:
C. Replacing one gas by another under the same conditions, has no effect on pressure.
Explanation:
Ideal gas:
A gas is treated as an ideal gas if temperature is high and pressure is low.
Kinetic energy for ideal gas given as
[tex]K.E.=\dfrac{3}{2}KT[/tex]
So when temperature of gas is increases then Average molecular kinetic energy will also increases.
The size of molecule is negligible as compare to the dimension of container. It mean that volume occupied by molecule is less as compare to the volume of container.
The between molecules is perfectly elastic.
Ideal gas equation
P V = m R T
So the option C is not always true.
Ideal gases are those gases in which no molecular attraction is present and following the ideal gas equation. Real gases are those that have molecular interaction, volume, and space. The correct option is:
Option C. Replacing one gas by another under the same conditions, has no effect on pressure.
Ideal gas is defined as the hypothetical gas that has no molecular interaction and occupies no space. The kinetic energy of the ideal gas can be expressed as:
- K.E. = [tex]\dfrac{3}{2}[/tex] KT
From the equation, it can be observed as the temperature of gas increases when the average kinetic energy increases. The size of the molecule is negligible when compared to the size of the container. The volume occupied molecule is less than compared to the volume of container. Thus, collision between molecules are elastic.
According to the ideal gas equation,
- PV = nRT
Therefore, the option C is not always true for the real gases.
To know more about ideal gas, refer to the following link:
https://brainly.com/question/13773584?referrer=searchResults
